An aqueous CdCl₂ solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Half-reaction at anode: Half-reaction at cathode: + + Standard Reduction Potentials (Volts) at 25 °C Cl₂(g) + 2 e 2 Cl-(aq) 1.360 O₂(g) + 4 H30+(aq) + 4 e¯ →→→ 6 H₂O(l) 1.229 2 H₂O(l) + 2 e² →→→ H₂(g) + 2 OH-(aq) -0.828 Cd²+ (aq) + 2 e² → Cd(s) -0.403 + + (b) What is the expected decomposition potential? + + + +
An aqueous CdCl₂ solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Half-reaction at anode: Half-reaction at cathode: + + Standard Reduction Potentials (Volts) at 25 °C Cl₂(g) + 2 e 2 Cl-(aq) 1.360 O₂(g) + 4 H30+(aq) + 4 e¯ →→→ 6 H₂O(l) 1.229 2 H₂O(l) + 2 e² →→→ H₂(g) + 2 OH-(aq) -0.828 Cd²+ (aq) + 2 e² → Cd(s) -0.403 + + (b) What is the expected decomposition potential? + + + +
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.50QE
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